Calculate the pH of a solution having `H^+` ion concentration `3.8xx10^-5m`.

Calculate the pH of a 0.2M solution of hydrocyanic acid (HCN). Ionisation constant (K_a) of HCN at 298K is 7.2xx10^(-10)

calculate the pH of a solution which is 0.1 m in CH_3COOH and .5 M in CH_3COONa . k_a for CH_3COOH is 1.8xx10^-6 .

Kohlrausch's law helps to determine the degree of dissociation of a weak electrolyte at a given concentration. The molar conductivity Lambda_m of .001M acetic acid is 4.95xx10^(_5)Scm^2mol^(-1) .Calculate the degree of dissociation (alpha) at this concentration if limiting molar conductivity lamda_m^0 for H+is 340xx10^(-5)Scm^2mol^(-1) and CH_3COO^- 50.5xx10^(-5)Scm^2mol^(-1)

The 'p' H of a solution is 5.9. If the hydrogen ion concentration is decerased hundred xx, the solution will be

At a certain temp, the dissociation constants of HCOOH and CH_(3)COOH are 1.8 times 10^(-4) and 1.8 times 10^(-5) respectively. The molarity of an CH_(3)COOH solution in which H^(+) concentration is the same as in a 0.001 M HCOOH solution is